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General Chemistry 111 > Chapter 9 > Flashcards

Chapter 9 Flashcards

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1
Q

what is a chemical bond

A

a strong attractive force that exists between neighboring atoms in a substance

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2
Q

three types of chemical bonds

A
  • ionic
  • covalent
  • metallic
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3
Q

what is a metallic bond

A

a regular arrangement of metal atoms, but the valence electrons move throughout the crystal

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4
Q

what is an ionic bond

A

a chemical bond formed by the electrostatic attraction between positive and negative ions

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5
Q

when do ionic bonds form

A

when one or more electrons are transferred from the valence shell of one atom to the valence shell of another atom

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6
Q

the atom that transfers electrons in ionic bonds

A

cation

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7
Q

the atom that gains electrons in an ionic bond

A

anion

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8
Q

G.N Lewis

A

introduced the Lewis Electron-Dot symbol to describe ions and molecules by considering a “cubical atom”

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9
Q

G.N Lewis and his hypothetical “cubical atom”

A

there is space for 8 electrons at the corners of a hypothetical cube

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10
Q

what did G.N Lewis recognize about atoms

A

there is a “kernel” of electrons that remain uncharged, and an outer shell that varies during chemical reactions between 0 and 8

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11
Q

valence electrons

A

the outer shell electrons of an atom. they are the electrons that participate in chemical bonding

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12
Q

Lewis’s Cubical Atom (definition)

A

a cube provides a simple means to illustrate valence electrons around an atom, but this is more commonly represented in 2-dimensions using “dots” to represent the valence electrons

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13
Q

Lewis dot symbol

A

a notion in which the electrons in the valence shell of an atom or ion are represented by dots placed around the chemical symbol of the element

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14
Q

how are lewis dot symbols placed

A

dots are placed one to a side until all 4 sides are occupied

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15
Q

what concept did Lewis introduce

A

the electron-pair bond and the “group of 8” electrons being the favorable situation

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16
Q

what did Lewis’s concept lead to

A

-the octet rule

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17
Q

octet rule definition

A

-molecules or ions tend to be most stable when the outermost electron shells contain 8 electrons and have structures that are isoelectronic with the noble gasses

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18
Q

what does the combination of ionization energy and electron affinity need

A

it needs energy because it is endothermic

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19
Q

lattice energy

A

the change in energy when an ionic solid is separated into gas-phase ions

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20
Q

what happens when 2 ions bond

A

energy is released, making the overall process exothermic

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21
Q

according to Coulombs law, what 2 factors affect the strength of the ionic bond

A
  • charge (Q)

- size of the ions

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22
Q

Coulomb’s Law

A

the energy (E) obtained in bringing 2 ions with electric charges Q+ and Q- from infinite separation to a distance (r) apart

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23
Q

equation for coulomb’s law

A

E=(Q+ x Q-)/r

24
Q

Q+

A

the charge on the cation

25
Q

Q-

A

the charge on the anion

26
Q

r

A

the distance between the ions

27
Q

what does solving for E in coulomb’s law give you

A

the strength of the ionic bond

28
Q

ionic substances are typically ________ solids

A

high-melting

29
Q

what 2 factors affect the strength of the ionic bond (Melting point: Coulomb’s Law

A

melting point (strength of ionic bond) increases as Q increases and/or as r decreases

30
Q

covalent bond

A

a chemical bond formed by sharing a pair of electrons

31
Q

how do we understand how covalent bonds form

A
  • we monitor the energy of two isolated hydrogen atoms as they move closer together
  • the energy decreases, first gradually and then more steeply, to a minimum
  • as the atoms continue to move closer, energy starts to increase dramatically because the nuclei repel
32
Q

bond length

A

the distance between the atoms when energy is at a minimum

33
Q

what is the importance of the Born-Haber Cycle

A

because it is very difficult to measure the lattice energy directly, using the energy changes for steps helps make it easier and gives the same result

34
Q

Orbitals

A

a place to put electrons

35
Q

Elements to the left of carbon have __________ and those to the
right have ________

A

empty orbitals

filled orbitals (lone pairs)

36
Q

coordinate covalent bond

A

is one where a single atom provides

both electrons

37
Q

Bond Lengths sorted by size

A

Triple bond < Double Bond < Single Bond

38
Q

Ionization energy and electron affinity provide

A

an
indication of how readily an atom may want to give up or
accept an electron

39
Q

Electronegativity is considered to be

A

the ability of an atom

in a molecule to attract electrons to itself.

40
Q

Linus Pauling

A

quantified the concept of electronegativity by comparing the
bond energy of a heteronuclear A-B bond with the corresponding
homonuclear A-A and B-B bond energies.

41
Q

The bond energy E(A-B) for a molecule A-B is always

A

greater than

the mean of the bond energies

42
Q

Pauling argued that the excess bond energy is due to the

A

ionic

component caused by the partial charges on the atoms in AB.

43
Q

Electron Affinity versus Electronegativity

A

Electron Affinity: measurable, Cl is highest.

Electronegativity is the ability of an atom to attract toward
itself the electrons in a chemical bond.
Electronegativity: relative, F is highest

44
Q

when the difference in electronegativity is 0

A

the bond is covalent

45
Q

when the difference in electroegativity is greater than or equal to 2

A

the bond is ionic

46
Q

when the difference in electronegativity is between 0 and 2

A

the bond is polar covalent

47
Q

Formal charge results from assuming

A

equal sharing of the

bonding electrons

48
Q

The formal charge on an atom in a Lewis dot structure is

determined by inspecting

A

how many lone pairs are present and

how many bonds it forms.

49
Q

The sum of the formal charges of the atoms in a molecule or ion
must equal

A

the charge on the molecule or ion.

50
Q

Resonance

A

means that the actual structure is a composite or an

average of the two structures.

51
Q

classic example of “resonance”.

A

benzene

52
Q

A “circle” is used to depict the fact that

A

the bonding cannot be
properly represented by a single Lewis structure in which a
“line” represents a shared electron pair bond

53
Q

Exceptions to the Octet Rule

A
  1. The incomplete octet
    (hypovalent or electron deficient molecules).
  2. Odd-electron molecules
  3. Hypervalent molecules (“valence shell expansion”)
54
Q

Bond order

A

is the number of pairs of electrons in a bond.

55
Q

bond energy

A

The enthalpy change required to break a particular bond into one mole of
gaseous molecules

56
Q

Bond energy is a measure of

A

bond strength: the greater the bond energy,

the stronger the bond, the more stable the molecule

57
Q

Bond energies can be used to estimate the

A

enthalpy change, ΔH, for a

reaction

General Chemistry 111 (8 decks)

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